1 .		Which of the following acids, if in solutions of equal concentration, is the most acidic? Online Text [Hint]
2 .		Which one of the following is the weakest acid? Online Text [Hint]
3 .		Lactic acid, HC3H5O3, has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka. Online Text [Hint]
4 .		Phenol is a weak acid with one acidic hydrogen. The pH of a 0.00500 M solution of phenol is 6.09. Calculate Ka. Online Text [Hint]
5 .		A 0.200 M solution of a weak acid, HX, is 9.4 percent ionized. Using this information, calculate Ka for HX. Online Text [Hint]
6 .		Calculate the pH of a 0.025 M solution of propanoic acid (Ka = 1.3 x 10-5). Online Text [Hint]
7 .		Barbital is a weak monoprotic acid with Ka = 1.0 x 10-8. What is the pH of a 1.5 x 10-4 M solution of barbital? Online Text [Hint]
8 .		The active ingredient in aspirin is acetylsalicylic acid, HC9H7O4, a monoprotic acid with Ka = 3.3 x 10-4 at 25°C. What is the pH of a solution obtained by dissolving two aspirin tablets, each containing 325 mg of acetylsalicylic acid in 100. mL of water? Online Text [Hint]
9 .		Hydroxylamine, HONH2, is a weak base. Write the Kb expression for hydroxylamine. Online Text [Hint]
10 .		Determine the pH of a 0.15 M H2NNH2 solution (Kb for H2NNH2 is 8.5 x 10-7). Online Text [Hint]
11 .		Calculate the molar concentration of OH- ions in a 0.050 M solution of ethylamine, C2H5NH2, (Kb = 6.4 x 10-4). What is [OH-] and the pH of this solution? Online Text [Hint]
12 .		The pH of a 0.25 M solution of base, B, is 9.10. Calculate the Kb for base B. Online Text [Hint]
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